How does Sodium acetate react with water?

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The discussion centers on the hydrolysis of sodium acetate in water, where the acetate ion (CH3COO-) interacts with water to produce acetic acid (CH3COOH) and hydroxide ions (OH-), resulting in an alkaline solution. This reaction exemplifies the Brønsted–Lowry acid-base theory. A 0.01M solution of sodium acetate can achieve a pH of 8.4, demonstrating that significant alkalinity can be observed even at low concentrations. The conversation also notes a decline in precise knowledge regarding these chemical processes over recent years.
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When sodium acetate CH3COONa reacts with water does it form hydroxide ions, leaving the neutralised solution alklain?
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Removes a 'proton' from the water molecule. You might think of it like, CH3COO-is the anion of a weak acid and Na+ is the cation of a strong base. Sodium acetate dissolved in water would if conc. is high enough, make the solution alkaline.
 
Congratulations, you just discovered process of hydrolysis :wink:

Yes, that's what is happening:

CH3COO- + H2O ↔ CH3COOH + OH-

You might want to read on Brønsted–Lowry acid–base theory, this reaction is an important part of it.
 
symbolipoint said:
Sodium acetate dissolved in water would if conc. is high enough, make the solution alkaline.

0.01M solution of sodium acetate has a calculated pH of 8.4, you don't need high concentrations for the effect to be easily observable.
 
Borek said:
0.01M solution of sodium acetate has a calculated pH of 8.4, you don't need high concentrations for the effect to be easily observable.
Some fading of precise knowledge has been happening the last several years. (That is, in my knowledge)
 
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